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the process by which molecules go from liquid to gaseous state; endothermic because gas has more energy than liquid, so energy must go into the system

Boiling

gas is able to come up from the bottom; occurs throughout entire liquid

Vapor Pressure

ability of molecules to enter vapor stage

Boiling Point

temperature at which vapor pressure of liquid is equal to the atmospheric pressure

Normal Boiling Point

temperature at which the vapor pressure of the liquid is equal to the normal atomospheric pressure

Temperature

a measure of the average kinetic energy

Relationship Between Temperature and Vapor Pressure

as temperature increases, energy of molecules increase. higher energy means less energy has to be added to become gaseous, so it is easier to become gaseous. higher ability to become gaseous = higher vapor pressure.as temp increases so does vapor pressure

Why does evaporation lower a liquid's temperature?

evaporation is endothermic, so energy enters the system and increases the molecules' energy. the energetic molecules evaporate, leaving low-energy molecules (not enough energy to become gas). lower energy is reflected in a lower temperature.

Melting Point

point where the liquid and solid have identical vapor pressures

Normal Melting Point

temperature at which the solid and liquid states have the same vapor pressure under conditions where the total pressure is one atmosphere

two or more elements physically sharing the same space; the elements' appearances may change, but their chemical properties won't; a mixture can be separated into its component parts with relative ease

Compound

two or more elements chemically combined; a new substance is formed and the individual elements lose their original properties

Homogenous

consistent throughout; components are evenly dispersed

Solution

a homogenous mixture

Solubility

the ability to dissolve

Temperature's Effect on Solubility

increases solubililty in solids and liquids; decreases solubility in gases

Pressure's Effect on Solubility

increases solubility in gases; no effect in solids/liquids

Why is it beneficial to have measures of concentration that are Temperature Independent?

temperature affects volume, but not mass. molality, mole fraction, & mass percent are mass-based, but molarity is volume-based. M of a solution may change as the temp. changes, but m, x, and m% won't change

Explain nature of solute and solvent in relation to (delta)T.

(delta)T doesn't depend on the nature of the solute, just on the number of solute particles (i); it does however depend on the nature of the solvent, because Kb and Kf are specific to each individual solvent.

Colligative Properties

properties that change when a solute dissolves in a solvent; vapor pressure, osmotic pressure, freezing point, boiling point

Enthalpy of Vaporization

(delta)Hvap; energy required to vaporize one mole of molecules at standard atmospheric pressure

Enthalpy of Fusion

(delta)Hfus; energy required to melt one mole of molecules at standard atmospheric pressure

Conjugate Base

everything that remains of the acid molecule after a proton is lost

Conjugate Acid

formed when the proton is transferred to the base; essentially base + H+

Conjugate Acid-Base Pair

two substances related to each other by the donating and accepting of a single proton; two substances that differ only by the presence or lack of H+; e.g., acid and conjugate base

Acid-Base Reaction

H+ and OH- combine to form H2O; also called neutralization reaction; enough base is added to react exactly with the acid in a solution

Precipitation Reaction

a reaction in which an insoluble substance forms and separates from the solution

Oxidation-Reduction (Redox) Reaction

a reaction in which one or more electrons are transferred

Equivalence Point

point in titration where enough titrant has been added to neutralize the base